Chapter 13: Problem 17
The catenation tendency \(\mathrm{C}, \mathrm{Si}\) and \(\mathrm{Ge}\) is in the order \(\mathrm{Gc}<\mathrm{Si}<\mathrm{C}\). The bond energics (in \(\mathrm{kJ} \mathrm{mol}^{-1}\) ) of \(\mathrm{C}\) C, Si Si and Ge Ge bonds respectively are (1) \(167,180,348\) (2) \(180,167,348\) (3) \(348,167,180\) (4) \(348,180,167\)
Short Answer
Expert verified
(3) 348, 167, 180
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Bond Energy
Bond energy is a measure of the strength of a chemical bond. It represents the energy required to break one mole of bonds in a substance in the gas phase. A higher bond energy indicates a stronger bond.
The bond energy is crucial for determining the catenation tendency of elements like carbon (C), silicon (Si), and germanium (Ge).
For example, carbon has a significantly higher bond energy compared to silicon and germanium. This is why carbon tends to form more stable and stronger bonds with itself.
To compare effectively, remember:
The bond energy is crucial for determining the catenation tendency of elements like carbon (C), silicon (Si), and germanium (Ge).
For example, carbon has a significantly higher bond energy compared to silicon and germanium. This is why carbon tends to form more stable and stronger bonds with itself.
To compare effectively, remember:
- The higher the bond energy, the stronger the bond.
- Stronger bonds contribute to higher catenation tendencies.
Stability of Compounds
The stability of a compound is directly related to the bond energy of the bonds within the compound. Higher bond energies usually mean more stable compounds. This is especially true for elements capable of catenation, as they form chains or rings with themselves.
Carbon is a prime example. With its high bond energy for C-C bonds, it forms very stable compounds, including complex structures like chains and rings. The lower bond energies of Si-Si and Ge-Ge bonds result in less stable structures when these elements form bonds with themselves.
In general, for elements capable of catenation, compound stability is influenced by:
Carbon is a prime example. With its high bond energy for C-C bonds, it forms very stable compounds, including complex structures like chains and rings. The lower bond energies of Si-Si and Ge-Ge bonds result in less stable structures when these elements form bonds with themselves.
In general, for elements capable of catenation, compound stability is influenced by:
- Bond strength (bond energy).
- The ability to form multiple bonds.
- The overall arrangement and interaction of atoms within the compound.
C-C Bonds
C-C bonds, or carbon-carbon bonds, are among the strongest single bonds in organic chemistry. The high bond energy (348 kJ/mol) means that these bonds are exceptionally strong and provide great stability to carbon-based compounds.
These bonds enable carbon to form a variety of structures, from simple hydrocarbons to complex biomolecules. The ability of carbon to catenate, or form long chains and rings, is a direct result of these strong C-C bonds. This makes carbon unique among other group 14 elements like silicon and germanium.
Key points about C-C bonds:
These bonds enable carbon to form a variety of structures, from simple hydrocarbons to complex biomolecules. The ability of carbon to catenate, or form long chains and rings, is a direct result of these strong C-C bonds. This makes carbon unique among other group 14 elements like silicon and germanium.
Key points about C-C bonds:
- High bond energy results in strong bonds.
- Facilitates the formation of complex and diverse structures.
- Contributes significantly to the stability and versatility of organic compounds.
Si-Si Bonds
Si-Si bonds, or silicon-silicon bonds, have a bond energy of 180 kJ/mol. This is lower than the bond energy for C-C bonds but higher than Ge-Ge bonds. Consequently, Si-Si bonds are less strong and stable compared to C-C bonds.
While silicon can also form chains and networks, its ability to catenate is limited compared to carbon. This is because the stability of these chains and networks is lower due to the weaker Si-Si bonds.
Important aspects of Si-Si bonds:
While silicon can also form chains and networks, its ability to catenate is limited compared to carbon. This is because the stability of these chains and networks is lower due to the weaker Si-Si bonds.
Important aspects of Si-Si bonds:
- Lower bond energy than C-C bonds but higher than Ge-Ge bonds.
- Results in moderate-strength bonds, less conducive to forming long, stable chains.
- Limits the diversity and complexity of silicon-based compounds.
Ge-Ge Bonds
Ge-Ge bonds, or germanium-germanium bonds, have the lowest bond energy (167 kJ/mol) among the group 14 elements discussed. This low bond energy means that Ge-Ge bonds are the weakest and least stable.
The low stability of Ge-Ge bonds greatly reduces the catenation tendency of germanium. As such, germanium is less likely to form long chains or complex structures compared to carbon and silicon.
Key characteristics of Ge-Ge bonds:
The low stability of Ge-Ge bonds greatly reduces the catenation tendency of germanium. As such, germanium is less likely to form long chains or complex structures compared to carbon and silicon.
Key characteristics of Ge-Ge bonds:
- Lowest bond energy among C, Si, and Ge bonds.
- Weakest and least stable bonds.
- Significantly limits the ability of germanium to form diverse and complex compounds.
